If $E_{op}^o$ for this electrode is $1.30\,volt$ then what will be the oxidation electrode potential at $pH = 3$ ? .............. $\mathrm{volt}$
${{\text{E}}_{op}}=\text{E}_{o\text{p}}^{o}-0.059\,\,{{\log }_{10\,}}\left[ {{\text{H}}^{+}} \right]$
$=\text{E}_{\text{op}}^{o}+0.059\times \text{pH}$
${=1.3+0.059 \times 3}$
${=1.33+0.177}$
${=1.477}$
${=1.48\, \mathrm{Volt}}$
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Statement $(I)$: A solution of $\left[\mathrm{Ni}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{2+}$ is green in colour.
Statement $(II)$: A solution of $\left[\mathrm{Ni}(\mathrm{CN})_4\right]^{2-}$ is colourless.
In the light of the above statements, choose the most appropriate answer from the options given below:
(image)
The transition temperature for $\alpha$ to $\beta$ phase change is $600 \mathrm{~K}$ and $C_{p, \beta}-C_{p, \alpha}=1 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$. Assume $\left(C_{p, \beta}-C_{p, \alpha}\right)$ is independent of temperature in the range of 200 to $700 \mathrm{~K} . \mathrm{C}_{p, \alpha}$ and $C_{p, \beta}$ are heat capacities of $\alpha$ and $\beta$ phases, respectively.
($1$)The value of entropy change, $\mathrm{S}_\beta-\mathrm{S}_\alpha$ (in $\mathrm{J} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$ ), at $300 \mathrm{~K}$ is. . . . . . .
[Use : $\ln 2=0.69$ Given : $S_\beta-S_\alpha=0$ at $\left.0 \mathrm{~K}\right]$
($2$) The value of enthalpy change, $\mathrm{H}_\beta-\mathrm{H}_\alpha$ (in $J$ mol ${ }^{-1}$ ), at $300 \mathrm{~K}$ is
Give the answer quetion ($1$) and ($2$)
| Element | $IE_1$ | $IE_2$ | $IE_3$ |
| $P$ | $495.8$ | $4562$ | $6910$ |
| $Q$ | $737.7$ | $1451$ | $7733$ |
| $R$ | $577.5$ | $1817$ | $2745$ |
Then incorrect option is